1. Fill in the table below
Description/Beginning of Sentence
1. As one goes down the vertical column in a given
family in the Periodic Table, the radius of the atom
2. As one goes from left to right in the same period of
the Periodic Table, the radius of the atom
3. The size of the atom gets bigger as one goes down a
column of a given group in the Periodic Table
because the number of principal energy levels
4. The size of the atom gets bigger as one goes down a
column of a given group in the Periodic Table
because the number of inner electrons
5. The size of the atom gets bigger as one goes down the
column of a group on the Periodic Table because the
attraction of the outer electrons to the nucleus is
reduced by the
6. The reduction of the attractive force between the
outer electrons and the nucleus due to the inner
electrons is called the
7. Within a given period, as the atomic number
increases, the size of the atom
8. As one goes from left to right on the Periodic Table,
the atomic number increases because of an increase in
the number of
9. As one goes from left to right across a period, the
atomic radius decreases because of the increased
attraction of the electrons by an increased number of
10. This describes the attraction of electrons toward the
nucleus, drawing them closer to the nucleus
11. The energy needed to remove an electron from an
atom is called
12. As one moves down a group, the ionization energy
needed to remove an electron to form an ion
13. As one moves down a group, the reason that the
ionization energy decreases, making it easier to
remove an electron is that the electrons are farther
from the
14. As one moves down a group, the reason the
ionization energy decreases, making it easier to
remove an electron is that there is an increase in
15. As one moves left to right across a period, the
ionization energy needed to remove an electron tends
to
16. As one moves left to right across a period, the
ionization energy needed to remove an electron
increases because there is an increase in
17. The tendency of an atom to attract other electrons to
itself is referred to as
18. As one moves down a group, the electronegativity
Answer/End of
Sentence
19. As one moves left to right across a period, the
electronegativity
20. These elements are an exception to the increase of
electronegativity from left to right across the Periodic
Table
21. These 2 things tend to increase as one moves down a
group on the Periodic Table
22. These 2 things tend to decrease as one moves down a
group on the Periodic Table
23. These 3 things tend to increase as one moves left to
right across a period on the Periodic Table
24. This tends to decrease as one moves left to right
across a period on the Periodic Table
25. These 2 things tend to remain constant as one moves
left to right across the Periodic Table
2. Respond to the questions below:
a. Where are the most active metals located?
b. Where are the most active nonmetals located?
c. As you go left to right across a period, what does atomic size do and why?
d. As you travel down a group, what does atomic size do and why?
e. How does a negative ion compare in size to its parent atom?
f. How does a positive ion compare in size to its parent atom?
g. As you go from left to right across a period, what does ionization energy do and why?
h. As you go down a group, what does ionization energy do and why?
i. Where is the highest electronegativity found?
j. Where is the lowest electronegativity found?
k. Elements of Group 1 are called…
l. Elements of Group 2 are called…
m. Elements of Groups 3 to 12 are called…
n. Where are the metals located? Nonmetals?
o. Elements of Group 17 are called…
p. The most active element in Group 17 is…
q. Elements of Group 18 are called…
r. What sublevels are filling across the transition elements?
s. What sublevels are filling in the first two groups of representative elements?
t. What sublevels are filling across the last 6 groups of representative elements?
u. What sublevels are filling in the bottom 2 rows on the Periodic Table (lanthanide and actinide
series)?
v. Elements within a group have a similar number of …
w. Elements across a period have a similar number of …
x. A colored ion generally indicates a …
y. As you go down a group, what happens to the metallic character of elements and why?
z. What is an element with both metallic and nonmetallic properties called and where would one be
located on the Periodic Table?
3. Respond to the following questions:
a. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
b. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
c. Why does fluorine have a higher ionization energy than iodine?
d. Why do elements in the same group tend to behave similarly in chemical reactions?
e. Rank in order of increasing atomic radius: K, Na, Rb.
f. Rank in order of increasing atomic radius: Br, I, F.
g. Rank in order of increasing atomic radius: N, O, F.
h. Rank in order of increasing atomic radius: Zr, Ru, Ag.
i. Explain the trend for atomic radius going across the periods of the Periodic Table.
j. Explain the trend for atomic radius going down the groups of the Periodic Table.
k. Rank in order of increasing ionization energy: Ca, Mg, Ra.
l. Rank in order of increasing ionization energy: Cr, W, Mo.
m. Rank in order of increasing ionization energy: Al, P, Si.
n. Rank in order of increasing ionization energy: Xe, Te, Sn.
o. Explain the trend for ionization energy going across the periods.
p. Explain the trend for ionization energy going down the groups.
q. Rank in order of decreasing electronegativity: Li, Na, Cs.
r. Rank in order of decreasing electronegativity: Si, Cl, P.
s. Rank in order of decreasing electronegativity: Se, Br, Kr.
t. Rank in order of decreasing electronegativity: F, B, C.
u. Explain the trend for electronegativity going across the periods.
v. Explain the trend for electronegativity going down the groups.
w. Rank in order of decreasing ionic radius: Be, Sr, Mg.
x. Rank in order of decreasing ionic radius: Cl, F, I.
y. Explain the trend for ionic size going across the periods.
z. Explain the trend for ionic size going down the groups.
aa. Explain why cations of an element tend to be smaller than their corresponding atoms.
bb. Explain why anions of an element tend to be larger than their corresponding atoms.
4. Periodic Table Review
a. Arrange the following elements in terms of increasing first ionization energy: He, K, Cl, Ar, Mg,
Ne
b. Why is the second ionization energy always larger than the first?
c. List some properties of metals.
d. What happens to the radius of an atom as you go down a group?
e. What happens to the ionization energy as you go down a group?
f. Where in the Periodic Table would you find the most electronegative elements?
g. Where in the Periodic Table would you find the least electronegative elements?
h. Compare the radius of a positive ion to that of its parent atom.
i. List the following in terms of increasing ionic radius: Mg+2, Na+1, Al+3
j. List the following in terms of decreasing ionic radius: F-1, I-1, Te-2
k. Which elements in the Periodic Table have the highest ionization energies?
For additional practice:
Relevant section in book is all of Chapter 7
Additional practice problems can be found on p. 337 (39-43), p. 338 (51, 52, 56-58, 61-64), p. 339 (67-70, 82,
84, 85, 86), and p. 340 (87-90)